The free energy of an electrochemical cell is given by the equation: AG = -nFE Where: AG = Gibbs Free Energy change n = moles of electrons F = Faraday's constant E = cell voltage NOTE: Write AG as dG (with no spaces) for the answers below. In order to solve for the Faraday's constant, F, you must multiply both sides of the equation by the same expression: AG × = -nFE × The resulting equation is: F =
The free energy of an electrochemical cell is given by the equation: AG = -nFE Where: AG = Gibbs Free Energy change n = moles of electrons F = Faraday's constant E = cell voltage NOTE: Write AG as dG (with no spaces) for the answers below. In order to solve for the Faraday's constant, F, you must multiply both sides of the equation by the same expression: AG × = -nFE × The resulting equation is: F =
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Transcribed Image Text:The free energy of an electrochemical cell is given by the equation:
AG = -nFE
Where:
AG = Gibbs Free Energy change
n = moles of electrons
Faraday's constant
E = cell voltage
F
NOTE: Write AG as dG (with no spaces) for the answers below.
In order to solve for the Faraday's constant, F, you must multiply both sides of the equation by the same expression:
AG ×
= -nFE x
The resulting equation is:
F =
Transcribed Image Text:The Ideal Gas Law is given by the equation:
PV — пRT
Where:
P = pressure
V = volume
n = moles
T = temperature in Kelvin
In order to solve for the moles, n, you must multiply both sides of the equation by the same expression:
PV ×
= nRT ×
The resulting equation is:
n =
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